A concentration cell is one in which both half-cells contain exactly the same electrodes and electrolyte solution but differ in the concentration of electrolytes. Based on the sketch outlining such a cell, answer the questions below.   In which half-cell, A or B, will the concentration of Zn²⁺ DECREASE over time? Why? 2 In which of the following directions will the electrons flow in the cell? 3 What is the maximum number of volts that these cells can generate?

A voltaic cell is constructed, based on the Zn/Sn2+ ion reaction. Zn + Sn2+ → Zn2+ + Sn The standard cell potential is 0.626 V. What is the cell potential be when [Zn2+]=1.2 M and [Sn2+]=0.8 M ?

A voltaic electrochemical cell is constructed using the following reaction. The half-cell components are separated by a salt bridge. Cr(s) + 3FE3+(aq)Cr3+(aq) + 3F22+(aq) Write the reactions that take place at the anode and at the cathode, the direction in which the electrons migrate in the external circuit, and the direction the anions in the salt bridge migrate. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Enter the reaction that takes place at the anode. Include state symbols: + Enter the reaction that takes place at the cathode. Include state symbols: + In the external circuit, electrons migrate v the Cr electrode v the Fe3+, Fe2+ electrode. Anions migrate v the salt bridge the Fe3+, Fe2+ compartment. Submit from proach Show Tutor Steps to

13. Write the oxidation half reaction, the reduction half reaction, and the overall cell reaction for the following galvanic cell. Identify the anode and the cathode and state why you labeled the metals that way. (4) Zn (s) | Zn²+ (aq) || Cu²+ (aq) | Cu (s)